Question

Q. It takes 0.15 mole of CIO - to oxidize 12.6 g of chromium oxide of a specific formula to Cr207- - , CIO - becomes CI - - ...( - means negative charge)​

Answer 1

52×2+16×7

104+112

216

Hope it helps u❤

Answer 2

$C_{r} O_{2}$

Explanation:

CIO-  + $Cr_{x} O_{y}$ →  $Cr_{2} O_{7} ^{-2} + CL^{-}$

+1                             +6           -1

Given that,

The state of oxidation shifts to CIO- to CI-

= 1 - (-1)

= 2

Let's assume $Cr_{x} O_{y}$ be n

As we know,

The oxidation state change = No. of electrons transferred

It has to be the same in both the given cases. so,

6 - n = 2

∵ n = 4

As $Cr_{x} O_{y}$ is neutral, thus

4x - 2y = 0

∵  2x = y

Thus, $C_{r} O_{2}$ is the right option.

Learn more: Chemical formula

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